pH and pOH Calculations
1)
Determine the pH of a 0.0034 M HNO
3
solution.
2)
Determine the pOH of a 0.0034 M HNO
3
solution.
3)
Determine the pH of a 4.3 x 10
4
M NaOH solution.
4)
If a solution is created by adding water to 2.3 x 10
4
moles of NaOH and
4.5 x 10
6
moles of HBr until the final volume is 1 L, what is the pH of this
solution?
5)
Determine the pH of a 4.5 x 10
11
M NaOH solution.
6)
Why would we say that a solution with a H
+
concentration of 1.00 x 10
7
M
is said to be neutral.
If it contains acid, shouldn’t it be acidic?
For chemistry help, visit www.chemfiesta.com
© 2002 Cavalcade Publishing – All Rights Reserved
This preview has intentionally blurred sections. Sign up to view the full version.
View Full Document
pH and pOH Calculations 
Answers
1)
Determine the pH of a 0.0034 M HNO
3
solution.
pH = log[H
+
] = log(0.0034) = 2.47
2)
Determine the pOH of a 0.0034 M HNO
3
solution.
pH = log[H
+
] = log(0.0034) = 2.47
pOH = 14 – pH = 14 – 2.47 = 11.53
3)
Determine the pH of a 4.3 x 10
4
M NaOH solution.
pOH = log[OH

] = log(4.3 x 10
4
) = 3.37
pH = 14 – pOH = 14 – 3.37 = 10.63
4)
If a solution is created by adding water to 2.3 x 10
4
moles of NaOH and
4.5 x 10
6
This is the end of the preview.
Sign up
to
access the rest of the document.
 Fall '09
 JULIAKOVACS
 pH, Sodium hydroxide, 1 L, pOH Calculations

Click to edit the document details